Independent- Surface area of calcium carbonate Dependent- Amount of carbon dioxide produced (cm3) Controls- Amount of calcium carbonate (g) Volume of hydrochloric acid (ml) Same beaker Same concentration of HCl Same temperature of both HCl and CaCO3 It is important to keep the amount of calcium carbonate the same‚ because if there is more calcium carbonate‚ more carbon dioxide is going to be produced. The volume of hydrochloric acid is only going to affect the rate of the
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I. Introduction An acid-base titration is a method of neutralizing strong acids. Unbeknownst to many‚ acid-base titrations occur on a daily basis. Our stomachs use acid to help us digest our food – approximately .155 hydrochloric acid (HCl) with a pH of 2-3. When too much of this acid is formed in the stomach‚ heartburn and other discomfort occurs. This is when people grab for their antacids; these are bases that neutralize the excess acid in the stomach. Calcium carbonate‚ magnesium
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being successful because the activation energy will be attainable. Hypothesis: In a reaction between calcium carbonate and hydrochloric acid‚ the products calcium chloride‚ carbon dioxide and water are formed. I predict that the higher temperature of HCl acid‚ the higher the reaction rate will be‚ this is because at a higher temperature there will more fast-moving hydrochloric acid molecules per set volume. This means that there will be a higher chance of the calcium carbonate molecules colliding with
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difference in the amount of calcium carbonate in brown versus white chicken eggs. Background: Calcium carbonate (CaCO3) is a component of seashells and eggshells that gives them their strength and hardness. Because calcium carbonate is a base‚ it will react with acids to form a salt and water. The complete reaction of calcium carbonate with hydrochloric acid is: CaCO3 (s) + HCl (aq) ( CaCl2 (aq) + CO2 (g) + H2O (l) The portion of the shell that is not calcium carbonate does not react with acid
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Part A: Reaction #1A: Na2CO3(aq) + HCL(aq)(0.5m) H2CO3(g) + 2NaCl(l) H2O(l) + CO2(g) + 2NaCl(l) Observations: There was a formation of a gas and the liquid was clear. Reaction #2A: Na2CO3(aq) + NaCl(aq) Na2CO3(aq) + NaCl(aq) Observation: No reaction was observed. Reaction#3A: Na2CO3(aq) + CaCl2(aq) 2NaCl(aq) + CaCO3(s) Observations: The solution turned white and cloudy which is evidence that a perticipate was formed. Reaction #4A: NaOH(aq) + HCl(aq)(0.5m) H2O(l) + NaCl(aq) Observations:
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Topic 10 Rate of Reaction Part A Unit-based exercise Unit 36 An introduction to rate of reaction Fill in the blanks 1 concentration; time 2 instantaneous 3 a) the gaseous product / carbon dioxide evolved b) loss in mass 4 a) colorimeter b) standard alkali c) the gaseous product / carbon dioxide evolved 1 time to reach the opaque stage 5 transmittance; 6 hydroxide; titrimetric True or false 7 T In the oxidation of methanoic acid by bromine‚ the intensity of the orange colour of bromine
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Calcium in each solution to figure out how well this method is. As we know‚ Ca2+ can form precipitation with oxalate in form CaC2O4. H2O in basic solution. So‚ in this method we will slowly precipitate all Ca2+ in the solution with C2O42- in acidic HCl solution and slowly raise pH of the solution by thermal decomposition of Urea. Then‚ we will filter and dry the precipitation from the solution and mass the precipitation. After all we will calculate to figure out how much Ca in the precipitation‚ then
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temperature‚ concentration of a solution‚ and catalysts will be tested to determine how they influence the rate of reaction. Materials: 1. Goggles 2. Powdered calcium carbonate (CaCO3) 3. Metal scoop 4. Marble chips 5. Cold water 6. Hot water 7. Room temperature water 8. 1M hydrochloric acid (HCl) 9. 3 M HCl 10. Iron (III) chloride (FeCl3) 11. Sodium chloride (NaCl) 12. Calcium chloride (CaCl2 ) 13. Potassium nitrate (KNO3) 14. 0.3% hydrogen peroxide (H2O2) solution 15. 8 test tubes
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M.M :40 Note : all questions are compulsory . Section A Q.1 By what other name is the unit coulomb × volt ? 1 Q.2 What do the symbols { } { } mean in electric circuit? Q.3 Balance the reaction CuO + HCl → CuCl2 + H2O Q.4 Name the process in which plants release CO2 . Q.5 what is displacement reaction? Give an example of is displacement reactions? Q.6 Write the differences between Autotrophic and parasitic nutrition. Q.7 An electric
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single-displacement reaction | Zn + 2 HCl (aq) --> ZnCl2(aq) + H2(g) | 3. Black smoke occurs | decomposition reactions | 2 (H2O2)(aq) MnO2 2 (H2O) + (O2) | 4. reddish-brown deposit on the surface of iron; surface of the iron is found corroded; the blue solution turns light green | single-displacement reaction | Fe + CuSO4(aq) --> FeSO4 + Cu | 5. PbSO4 (milk white) | double-displacement reaction | Pb(NO3 )2(aq) + H2SO4(aq) --> PbSO4 + 2HNO3 | 6. CaCO3 (s) appears to dissolve
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